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The physics of cooling
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Recommended: The physics of cooling
Joseph Amoah-Tetteh
September 18, 2016
Lab 2 Specific Heat
Purpose:
Purpose for the lab is explore and observe the transfer of heat from a piece of metal to its surroundings and quantify the amount of thermal energy transferred. The first law of thermodynamics states that energy cannot be created nor broken down. In this experiment, water is heated with a metal and placed into water at room temperature. The results will be the heat change between the metal and the water at room temperature explaining that energy cannot be created nor destroyed.
Introduction:
Specific heat is the heat required to raise the temperature of the unit mass of a given substance by a given amount. Specific heat is another physical property of matter. All matter has a temperature associated with it. The temperature of matter is a direct measure of the motion of the molecules: The greater the motion the higher the temperature:
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Lab Data:
Room Temperature: 21.5 Celsius = 294.5 Kelvin
Mass of metal: 57 grams
Inner metal Cup + Stirrer Mass 67.2 grams
Inner metal Cup + Stirrer Mass + Water 250.3 grams
Room’s initial temperature is 22.4 Celsius
Boiling Temperature 88.1 Celsius
Final Temp of All Items 24.2 Celsius Calculations
Quantity Heat Equation: q = Quantity of Heat Transferred q = s x m x (Tf – Ti) s = Specific Heat g = Grams of Substance
Specific Heat Equation: Tf = Final Temperature s = ___q ___ Ti = Initial Temperature m x (Tf – Ti)
Specific Heat of Water = 4.184J
Sample 1 q = (4.184J)(57g)(22.4°C – 22.4°C) q = 235 J s = ___-235 ___
(1.33g)(21 C- 100 °C)
s = 2.023124
Thermodynamics is essentially how heat energy transfers from one substance to another. In “Joe Science vs. the Water Heater,” the temperature of water in a water heater must be found without measuring the water directly from the water heater. This problem was translated to the lab by providing heated water, fish bowl thermometers, styrofoam cups, and all other instruments found in the lab. The thermometer only reaches 45 degrees celsius; therefore, thermodynamic equations need to be applied in order to find the original temperature of the hot water. We also had access to deionized water that was approximately room temperature.
Tf-Ti). Next, subtract the initial temperature, 25 degrees from the final temperature, 29 degrees putting the change in temperature at 4 °C. To calculate the heat absorbed by the water in calorimeter, use the formula (q = mCΔT). Plug in 50 mL for (m), 4.184 J for (C) and 4 °C for the initial temperature (ΔT), then multiply.
Temp: Mass of evap. dish: Mass of evap dish+contents: Mass of contents: Solubility g/100cm3 water
Lab 4: Energy Conservation: Hot Stuff!! The purpose of this experiment is to try to find the original temperature of the hot water in the heater using the 60 degrees C thermometer. Use your 60°C thermometer, and any materials available in your laboratory, to determine the temperature of the water in the coffee pot. During this experiment we calculated the original temperature of a heater after it had been cooled down, and we did this by measuring hot, cold, and warm water, with a thermometer that had tape covering 60 degrees and up.
The purpose of this lab was to calculate the specific heat of a metal cylinder
When there is a heat exchange between two objects, the object’s temperature will change. The rate at which this change will occur happens according to Newton’s Law of heating and cooling. This law states the rate of temperature change is directly proportional between the two objects. The data in this lab will exhibit that an object will stay in a state of temperature equilibrium, unless the object comes in contact with another object of a different temperature. Newton’s Law of Heat and Cooling can be understood by using this formula:
The first law of thermodynamics simply states that heat is a form of energy and heat energy cannot be created nor destroyed. In this lab we were measuring the change in temperature and how it affected the enthalpy of the reaction.
Variables --------- During the experiments, the water will be heated using different spirit burners containing different alcohols. I will be able to change different parts of the experiment. These are the. Volume of water heated:
The purpose of performing this lab was to find the specific heat capacity of an unknown metal.
water has had equal amounts of time for it to heat up, again I will
Specific heat capacity of aqueous solution (taken as water = 4.18 J.g-1.K-1). T = Temperature change (oK). We can thus determine the enthalpy changes of reaction 1 and reaction 2 using the mean (14) of the data obtained. Reaction 1: H = 50 x 4.18 x -2.12.
The objective of this experiment was to identify a metal based on its specific heat using calorimetry. The unknown metals specific heat was measured in two different settings, room temperature water and cold water. Using two different temperatures of water would prove that the specific heat remained constant. The heated metal was placed into the two different water temperatures during two separate trials, and then the measurements were recorded. Through the measurements taken and plugged into the equation, two specific heats were found. Taking the two specific heats and averaging them, it was then that
Conduction, Convection, and Radiation Heat transfer is the way heat moves through matter to change the temperature of other objects. There are three types of heat transfers, Conduction, Convection, and Radiation. The first kind of heat transfer, conduction, is heat transferring through direct contact of materials. This would be the same thing as a pan on the stove. The heat from the stove touches the pan directly, therefore making the pan hot.
- Temperature was measured after and exact time i.e. 1 minute, 2 minutes, 3 minutes.
Thermodynamics is the branch of science concerned with the nature of heat and its conversion to any form of energy. In thermodynamics, both the thermodynamic system and its environment are considered. A thermodynamic system, in general, is defined by its volume, pressure, temperature, and chemical make-up. In general, the environment will contain heat sources with unlimited heat capacity allowing it to give and receive heat without changing its temperature. Whenever the conditions change, the thermodynamic system will respond by changing its state; the temperature, volume, pressure, or chemical make-up will adjust accordingly in order to reach its original state of equilibrium. There are three laws of thermodynamics in which the changing system can follow in order to return to equilibrium.